Complete Whole Notebook

More documents

Recommendations

Info

Learning Goal for this section: Explain and compare nuclear reactions (radioactive decay, fission and fusion), the energy changes associated with them and their associated safety issues. Notes Section: Nucleus= protons+neutrons N-1amu-0 / (+,-) P-1amu-+ E-none- - Element 10 has 20 isotopes All living things are made up of carbon Bottom of periodic table- the mass gets massive Isotopes are an element or atom that has a diferent mass than neutrons It becomes stable when the number of protons are equal or similar to the number of neutrons When the particles are connected to your cells it becomes cancerous Beta particles have a mass of an electron You are able to convert neutrons to protons Unit is AMU for protons and neutrons Gamma radiation can kill Gamma radiation is energy More dense the more the atoms are together Gamma radiation is associated with radioactive decay 54
The Nucleus A typical model of the atom is called the Bohr Model, in honor of Niels Bohr who proposed the structure in 1913. The Bohr atom consists of a central nucleus composed of neutrons and protons, which is surrounded by electrons which “orbit” around the nucleus. Protons carry a positive charge of one and have a mass of about 1 atomic mass unit or amu (1 amu =1.7x10- 27 kg, a very, very small number). Neutrons are electrically “neutral” and also have a mass of about 1 amu. In contrast electron carry a negative charge and have mass of only 0.00055 amu. The number of protons in a nucleus determines the element of the atom. For example, the number of protons in uranium is 92 and the number in neon is 10. The proton number is often referred to as Z. Atoms with different numbers of protons are called elements, and are arranged in the periodic table with increasing Z. Atoms in nature are electrically neutral so the number of electrons orbiting the nucleus equals the number of protons in the nucleus. Neutrons make up the remaining mass of the nucleus and provide a means to “glue” the protons in place. Without neutrons, the nucleus would split apart because the positive protons would repel each other. Elements can have nucleii with different numbers of neutrons in them. For example hydrogen, which normally only has one proton in the nucleus, can have a neutron added to its nucleus to from deuterium, ir have two neutrons added to create tritium, which is radioactive. Atoms of the same element which vary in neutron number are called isotopes. Some elements have many stable isotopes (tin has 10) while others have only one or two. We express isotopes with the nomenclature Neon-20 or 20 Ne 10, with twenty representing the total number of neutrons and protons in the atom, often referred to as A, and 10 representing the number of protons (Z). Alpha Particle Decay Alpha decay is a radioactive process in which a particle with two neutrons and two protons is ejected from the nucleus of a radioactive atom. The particle is identical to the nucleus of a helium atom. Alpha decay only occurs in very heavy elements such as uranium, thorium and radium. The nuclei of these atoms are very “neutron rich” (i.e. have a lot more neutrons in their nucleus than they do protons) which makes emission of the alpha particle possible. After an atom ejects an alpha particle, a new parent atom is formed which has two less neutrons and two less protons. Thus, when uranium-238 (which has a Z of 92) decays by alpha emission, thorium-234 is created (which has a Z of 90). Because alpha particles contain two protons, they have a positive charge of two. Further, alpha particles are very heavy and very energetic compared to other common types of radiation. These characteristics allow alpha particles to interact readily with materials they encounter, including air, causing many ionizations in a very short distance. Typical alpha particles will travel no more than a few centimeters in air and are stopped by a sheet of paper. 55
Page 1 and 2:
Bryan’s Chemistry Notebook
Page 3 and 4:
Unit 1 Measurement Lab Separation o
Page 5 and 6: Unit 5 (28 days) Chapter 10 Chemica
Page 7 and 8: 30. Always lubricate glassware (tub
Page 9 and 10: 7
Page 11 and 12: Print vs. print Online vs. online P
Page 13 and 14: To use the Stair-Step method, find
Page 15 and 16: Using SI Units Match the terms in C
Page 17 and 18: Standards of Measurement Fill in th
Page 19 and 20: SCIENTIFIC NOTATION RULES How to Wr
Page 21 and 22: Convert each number from Scientific
Page 23 and 24: Significant Figures Rules There are
Page 25 and 26: How Many Significant Digits for Eac
Page 27 and 28: The following rule applies for mult
Page 29 and 30: Learning Goal: Benchmark 1qt=32 oz
Page 31 and 32: Chapter 5 Electrons in Atoms The st
Page 33 and 34: Atoms Are Building Blocks Atoms are
Page 35 and 36: Electrovalence Don't get worried ab
Page 37: Summary
Page 40 and 41: The Learning Goal for this assignme
Page 42 and 43: In the space below, write the unabb
Page 44 and 45: Create groups for these Scientist a
Page 46 and 47: The Learning Goal for this Assignme
Page 48 and 49: Define Atomic Size: Atomic Size The
Page 50 and 51: Electronegativity Define Electroneg
Page 52 and 53: Unit 3 Chapter 25 Nuclear Chemistry
Page 54 and 55: Bryan Vega Name ___________________
Page 58 and 59: Beta Particle Decay Beta decay is a
Page 62 and 63: Ion Charge? What is the charge on f
Page 66 and 67: C 2 H 6 O Ethanol CH 3 CH 2 O Step
Page 68 and 69: Linear Molecular Geometry Orbital E
Page 70 and 71: Bent Molecular Geometry Orbital Equ
Page 72 and 73: Trigonal Pyramid Molecular Geometry
Page 74 and 75: Trigonal Bi Pyramid Molecular Geome
Page 76 and 77: Octahedral Molecular Geometry Orbit
Page 78 and 79: Orbitals Equation Lone Pairs Angle
Page 80 and 81: Chapter 9 Unit 4 Chemical Names and
Page 82 and 83: http://www.bbc.co.uk/education/guid
Page 84 and 85: Unit 5 Chapter 10 Chemical Quantiti
Page 86 and 87: The Mole LG:The students will learn
Page 88 and 89: LG:The students will learn how chem
Page 90 and 91: List what type the following reacti
Page 92 and 93: LG:The students will learn how chem
Page 94 and 95: Step 5 Balance the hydrogen atoms n
Page 96 and 97: 6) ___ Mn(NO2)2 + ___ BeCl2 ___ Be
Page 100 and 101: Stoichiometry and Balanced Equation
Page 102 and 103: Step 1: 200g C3H8 is equal to 4.54
Page 104 and 105: Stoichiometry and balanced equation
Page 106 and 107:
%yield = 6.1 tons × 100 = 64% 9.6t
Page 108 and 109:
Use the space provided to write out
Page 110 and 111:
Unit 6 Chapter 13 States of Matter
Page 112 and 113:
The Learning Goal for this assignme
Page 114 and 115:
13.3 The Nature of Solids A Model o
Page 116 and 117:
LG:The students will learn how gase
Page 118 and 119:
When the volume increases, the temp
Page 120 and 121:
Pg118
Page 122 and 123:
Water freezes at -0 o C Kelvin at 2
Page 124 and 125:
Combined gas Law- When we put Boyle
Page 126 and 127:
Page 128 and 129:
126 Unit 7 Chapter 16 Solutions The
Page 130 and 131:
Page 132 and 133:
Part 5: Molarity Molarity (M) is th
Page 134 and 135:
Page 136 and 137:
The Time-Temperature Graph We are g
Page 138 and 139:
Step Two: solid ice melts Now, we c
Page 140 and 141:
Step Four: liquid water boils Now,
Page 142 and 143:
The following table summarizes the
Page 144 and 145:
The Learning Goal for this section
Page 146 and 147:
2CO + O2 → 2CO2 6 If the above re
Page 148 and 149:
12 Which action will drive the reac
Page 150 and 151:
Unit 8 Chapter 19 Acid and Bases Th
Page 152 and 153:
The Learning Goal for this section
Page 154 and 155:
This would be a generic base: 152 X
Page 156 and 157:
HCl + H2O ⇌ H3O + + Cl¯ HCl - th
Page 158 and 159:
Several categories of substances ca
Page 160 and 161:
1. 2.82 2. 8.30 3. 0.00 4. 3.485 5.
Page 162 and 163:
Page 164 and 165:
2. What is the oxidation number of
Page 166 and 167:
One point of concern: notice that e
Page 168 and 169:
Reference Tables for Physical Setti
Page 170 and 171:
150. 140. Table G Solubility Curves
Page 172 and 173:
Table I Heats of Reaction at 101.3
Page 174 and 175:
Table O Symbols Used in Nuclear Che
Page 176 and 177:
0 6.941 +1 Li 3 2-1 Na 39.0983 K +1
Page 178 and 179:
First Atomic Symbol Name Ionization
Page 180 and 181:
Collier County CHEMISTRY EXAM FORMU
Page 182 and 183:
CHEMISTRY EXAM FORMULA AND RESOURCE
show all

Complete Whole Notebook

Create successful ePaper yourself

Delete template?

Save as template?